CSET Multiple Subject Subtest II Science Chemistry, Physics, and Astronomy

Chemistry

The science of the substances that make up our world.

The law of Conservation of mass

states that mass is neither created nor destroyed during ordinary chemical reactions or physical changes.

Matter

that which has mass and occupies space

Frenchman Lavoisier

French chemist known as the father of modern chemistry

Compounds

substances formed by the joining of elements through chemical bonding. every molecule of a compound is the same.

Atom

the smallest component of an element having the chemical properties of the element

John Dalton

English chemist and physicist who formulated atomic theory and the law of partial pressures

The Atomic Theory

1. Atoms are divisible

2. An element can have atoms with different masses.

Molecule

the simplest structural unit of an element or compound Composed of several bonded atoms.

Diatomic

of or relating to a molecule made up of two atoms

State of Matter

a physical property that describes matter as a solid, liquid, or gas

Solid

the state of matter in which the volume and shape of a substance are fixed. The retain their shape.

Liquid

a form of matter that flows, has constant volume, and takes the shape of its container but cannot be compressed.

Gas

the state of matter distinguished from the solid and liquid states by: relatively low density and viscosity and expand to fill any space.

Boyles Law

the law that states that for a fixed amount of gas at a constant temperature, the volume of the gas increases as the pressure of the gas decreases and the volume of the gas decreases as the pressure of the gas increases

Subatomic Particles

Protons, Neutrons, Electrons

Parts of an Atom

Nucleus: a very small region near the center of an atom. It contains protons and neutrons

Electrons: negatively charged particles surrounding the nucleus

Chemical Elements

substances that cannot be split into simpler substances by ordinary chemical means.

Atomic Number

equal to the number of protons in the nucleus or electrons in the neutral state of an atom of an element

The Chemical Nature of an Atom

The number of protons establishes this....

Nuetron

A small particle in the nucleus of an atom, with no electrical charge

Nuetral Atom

nuetral charge and equal number of protons and electrons

Charted Elements

In order of increasing atomic number in which a pattern of recurring physical and chemical properties is displayed.

Mendeleev

Russian chemist who developed a periodic table of the chemical elements and predicted the discovery of several new elements (1834-1907)

Naturally Occuring Elements

There are 91

Periodic Table

an arrangement of the elements in order of their atomic numbers so that elements with similar properties fall in the same column, or group

Bonds

The forces that hold molecules together. Can be covalent, ionic, hydrogen, etc.

Ions

A charged atom or group of atoms formed by the gain or loss of electrons.

Water

the most familiar of all liquids.

Solution

a homogeneous mixture of two or more substances

Acids

compounds that form hydrogen ions when dissolved in water

Bases (ALKALINE)

compounds that reduce the concentration of hydrogen ions in a solution

Electrolysis

The process of decomposing a chemical compound by the passage of an electric current.

Chemical Reaction

a process in which one or more substances are changed into others

Alkali Metals

the elements of Group 1 of the periodic table, lithium, sodium, potassium, rubidium, cesium, and francium.

Alloy

a combination; a mixture of two or more metals

Carbon Dioxide

a heavy odorless colorless gas formed during respiration and by the decomposition of organic substances, CO₂

Catalyst

(chemistry) a substance that initiates or accelerates a chemical reaction without itself being affected

Charles' Law

the law that states that for a fixed amount of gas at a constant pressure, the volume of the gas increases as the temperature of the gas increases and the volume of the gas decreases as the temperature of the gas decreases

Combustion

a process in which a substance reacts with oxygen to release heat and light

Compound

(chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight

Decomposition

A chemical reaction in which a compound is broken down into simpler compounds or elements.

Density

mass per unit volume of a substance.

Diffusion

the intermingling of molecules in gases and liquids as a result of random thermal agitation

Distillation

the process of purifying a liquid by boiling it and condensing its vapors

Electron

a negatively charged sub atomic particle; located outside the atomic nucleus Forms a cloud around the atomic nucleus. Electron movement constitutes electrical current.

Element

any of the more than 100 known substances (of which 92 occur naturally) that cannot be separated into simpler substances and that singlely or in combination constitute all matter

Evaporation

the process by which water changes from liquid form to an atmospheric gas

Freezing Point

the temperature below which a liquid turns into a solid

Hydrocarbons

organic molecules that are composed of only carbon and hydrogen

Hydrolysis

a chemical process in which a compound is broken down and changed into other compounds by taking up the elements of water.

Isotope

an atom that has the same number of protons (or the same atomic number) as other atoms of the same element do but that has a different number of neutrons (and thus a different atomic mass) Stable or Radioactive

Litmus

an paper indicator that is red in an acid and blue in a alkaline base

Mixture

(chemistry) a substance consisting of two or more substances mixed together not in fixed proportions and not with chemical bonding

Organic Compound

any compound of carbon and another element or a radical

Oxidation

A chemical change in which a substance combines with oxygen, as when iron oxidizes, forming rust.

pH

a value that indicated the acidity or alkalinity of a solution on a scale of 0-14, based on the proportion of H+ ions., p-otential of H-ydrogen

Proton

a subatomic particle with positive charge equal to the negative charge of an electron occuring in the atomic nucleus.

Saturated

being the most concentrated solution possible at a given temperature

Solute

the dissolved substance in a solution

Solvent

a liquid substance capable of dissolving other substances

Sublimination

going from gas to solid Example: dry ice= carbon dioxide Going from solid phase to gas phase

Synthesis

the process of producing a chemical compound usually by the union of simpler chemical compounds.

Physics

the science of matter and energy and their interactions.

The Scientific Method

1. Formulate a hypothesis that can be tested empirically. 2. Design the study and collect the data.3. Analyze the data and draw conclusions. 4. Report the findings. It requires observation, conjecture, calculation, prediction and testing.

Measurement

the beginning of scientific wisdom. Can it be measured?

A Unit

measurement

Kilo

one thousand grams

Kilometer

a metric unit of length equal to 1000 meters (or 0.621371 miles)

Millimeter

a metric unit of length equal to one thousandth of a meter

Meter

the basic unit of length adopted under the Systeme International d'Unites approximately 1.094 yards long

Liter

a metric unit of capacity equal to the volume of 1 kilogram of pure water at 4 degrees centigrade and 760 mm of mercury (or approximately 1.76 pints)

Gram

a metric unit of weight equal to one thousandth of a kilogram

Motion

describe by stating an ogjects position, velocity and acceleration.

Velocity

distance travelled per unit time

Acceleration

(physics) a rate of change of velocity

Newton's Laws

Law of Gravity. Inertia, Force, and Reaction

Law of Inertia

Law stating that objects at rest remain at rest and objects in motion continue in a straight line unless acted upon by a net external force.

Law of Force

law stating that strongly charged objects attract or repel other strongly charged objects, while weak objects have a weak effect upon other weak forces

Law of Reaction

for every action there is an equal and opposite reaction

Law of Gravity

all objects in the universe attract each other through gravitational force. Size of force depends on mass and distance

Energy

the ability to perform work, to move objects.

Potential Energy

Energy stored due to an object's position or arrangement

Kinetic Energy

the mechanical energy that a body has by virtue of its motion

Thermal Energy

the total kinetic and potential energy of all the particles in a substance.

Temperature

A measure of the average energy of motion of the particles in a substance

Sound

produced by the mechanical disturbance of a gas, liquid or solid.

Electricity

exists where the number of negative electrons does not precisely equal the number of positeve protons.

Magnetism

A property of some materials in which there is a force of repulsion or attraction between certain like and unlike poles.

Light

(physics) electromagnetic radiation that can produce a visual sensation

Theory of Relativity

..., Proposed by the Jewish physicist Albert Einstein (1879-1955) in the early part of the 20th century, is one of the most significant scientific advances of all time. Although the concept of relativity was not introduced by Einstein, his major contribution was the recognition that the speed of light in a vacuum is constant and an absolute physical boundary for motion.

Nuclear Energy

the energy released by a fission or fusion reaction; the binding energy of the atomic nucleus

Quantum Theory

the study of the structure and behavior of the atom and of subatomic particles from the view that all energy comes in tiny, indivisible bundles

Max Planck

German physicist whose explanation of blackbody radiation in the context of quantized energy emissions initiated quantum theory (1858-1947)

Absolute Zero

the lowest temperature theoretically attainable at which the kinetic energy of atoms and molecules is minimal 0 Kelvin or -273.15 Centigrade or -459.67 Fahrenheit

Buoyancy

The upward force on an object immersed in a fluid.

Calorie

unit of heat defined as the quantity of heat required to raise the temperature of 1 gram of water by 1 degree centigrade at atmospheric pressure

Capillarity

the attraction between molecules that results in the rise of a liquid in small tubes

Centrifugal

tending to move away from a center toward the perimeter

Centripetal

tending to move toward a center